Directions:
a) list and define all vocabulary from the chapter Ion- An element that has donated or taken electrons. Cation- Positive ions that gave away electrons. Anion- Negative charged ions that gained a pair of electrons. Monotomic Ion- An ion consisting of only one element. Polyatomic Ion- An ion composed of 2 or more elements. Ionic Bonds- Oppositely charged ions attract and bond to each other using each others electrons. Percent composition- Calculating the percentage of an element that exists within a compound. Empirical Formula- Gives the lowest whole-number ratio of the elements in the compound. Hydrates- compounds that have water trapped in them. Theoretical Percent- the amount of an element that is theorized to be within a compound without doing a lab.
b) type at least 4 sample problems with step-by-step directions of how to solve the problem; list the correct answers (if your chapter doesn't have math, there are still problems and concepts we learned.)
1) How many Valence Electrons does Phosphorus(P) have?
To solve the problem, you look at the periodic table, and find it's row. since it is in the fifth row from the left, you count over to find that it has 5 valence electrons.
2) Name this ionic compound- MgCO3 5H2O
by breaking up the first part, it is Magnesium and Carbonate. Then seeing that there are 5 H2O molecules it has the prefix, Penta and is finished with hydrate. You then get Magnesium Carbonate Pentahydrate.
3)Find the percent composition of H and O in H2O.
Start by finding the mass of each individual element. H: 2x1.01= 2.02 O:1x 15.99= 15.99
Add them together to get the entire mass of the compound. 2.02 + 15.99= 18.01
Divide each individual part of the compound by the total mass of the compound to find the percent composition for each.
H: 2.02/18.01= 0.112 --> 11.2% O: 15.99/18.01= 0.8878--> 88.78%
4) Find the percent composition of the water in the hydrate BaCl2 x 2H2O.
Start by finding the total atomic mass of the compound(all elements, including water). Ba-137.3g Cl- 2x35.45= 70.90g H2O- 2x18.01= 36.02
Total mass= 244.2g
Then divide the mass of the water by the total to get the percent of water in the hydrate. (36.02/244.2) x100= 14.75% H2O
c) link at least 3 websites for additional resources to help with studying
hyperphysics.phy-astr.gsu.edu/hbase/chemical/bond.html
www.chem.tamu.edu/class/majors/tutorialnotefiles/empirical.htm
www.sccs.swarthmore.edu/users/08/ajb/tmve/.../docs/Hydrate.html
d) develop your own LEQ questions for the section - what did you think were the key points we learned?
How are Ionic Bonds formed from monatomic and polyatomic ions?
How do you use percent composition and empirical formulas?
What makes a Hydrate different than a regular compound?
e) Once your page is done, visit 4 other chapters and answer their LEQ's. (This can be done on a separate piece of paper.)
a) list and define all vocabulary from the chapter
Ion- An element that has donated or taken electrons.
Cation- Positive ions that gave away electrons.
Anion- Negative charged ions that gained a pair of electrons.
Monotomic Ion- An ion consisting of only one element.
Polyatomic Ion- An ion composed of 2 or more elements.
Ionic Bonds- Oppositely charged ions attract and bond to each other using each others electrons.
Percent composition- Calculating the percentage of an element that exists within a compound.
Empirical Formula- Gives the lowest whole-number ratio of the elements in the compound.
Hydrates- compounds that have water trapped in them.
Theoretical Percent- the amount of an element that is theorized to be within a compound without doing a lab.
b) type at least 4 sample problems with step-by-step directions of how to solve the problem; list the correct answers (if your chapter doesn't have math, there are still problems and concepts we learned.)
1) How many Valence Electrons does Phosphorus(P) have?
To solve the problem, you look at the periodic table, and find it's row. since it is in the fifth row from the left, you count over to find that it has 5 valence electrons.
2) Name this ionic compound- MgCO3 5H2O
by breaking up the first part, it is Magnesium and Carbonate. Then seeing that there are 5 H2O molecules it has the prefix, Penta and is finished with hydrate. You then get Magnesium Carbonate Pentahydrate.
3)Find the percent composition of H and O in H2O.
Start by finding the mass of each individual element. H: 2x1.01= 2.02 O:1x 15.99= 15.99
Add them together to get the entire mass of the compound. 2.02 + 15.99= 18.01
Divide each individual part of the compound by the total mass of the compound to find the percent composition for each.
H: 2.02/18.01= 0.112 --> 11.2% O: 15.99/18.01= 0.8878--> 88.78%
4) Find the percent composition of the water in the hydrate BaCl2 x 2H2O.
Start by finding the total atomic mass of the compound(all elements, including water). Ba-137.3g Cl- 2x35.45= 70.90g H2O- 2x18.01= 36.02
Total mass= 244.2g
Then divide the mass of the water by the total to get the percent of water in the hydrate. (36.02/244.2) x100= 14.75% H2O
c) link at least 3 websites for additional resources to help with studying
hyperphysics.phy-astr.gsu.edu/hbase/chemical/bond.html
www.chem.tamu.edu/class/majors/tutorialnotefiles/empirical.htm
www.sccs.swarthmore.edu/users/08/ajb/tmve/.../docs/Hydrate.html
d) develop your own LEQ questions for the section - what did you think were the key points we learned?
How are Ionic Bonds formed from monatomic and polyatomic ions?
How do you use percent composition and empirical formulas?
What makes a Hydrate different than a regular compound?
e) Once your page is done, visit 4 other chapters and answer their LEQ's. (This can be done on a separate piece of paper.)